Electromagnetic Radiation- A form of energy that exhibits wavelike behavior as it travels through space
Quantum-Energy is the minimum quantity of energy that can be lost or gained by an atom.
Wavelength- λ-The distance between corresponding points on adjacent waves.
Frequency- ν-Defined as the number of waves that pass a given point in a specific time, usually one second. (wave/second) 1 w/s=Hertz
Speed of light: 3.00 x 108 meters/second
Frequency & Wavelength relationship:
Speed of light= wavelength X frequency
Photoelectric effect- Refers to the emission of electrons from a metal when light shines on the metal
Planck’s Constant: 6.626 x 10-34 Joules x Seconds
Relationship between a quantum of energy and frequency of radiation:
Energy= Planck’s constant X Frequency
Photon- A particle of electromagnetic radiation having zero mass and carrying a quantum of energy
When a narrow beam of the emitted light was shined through a prism, it was separated into 4 specific colors of the visible spectrum. 4 bands of lights were part of hydrogens line-emission spectrum.
Continuous Spectrum- The emission of a continuous range of frequencies of electromagnetic radiation.
Bohr Model:
· Electrons can have only certain energies
· Colors are emitted when electrons jump from higher to lower energy levels
Aufbau Principle: the principle that states that the structure of each successive element is obtained by adding one proton to the nucleus of the atom and one electron to the lowest-energy orbital that is available
Pauli Exclusion Principle: the principle that states that two particles of a certain class cannot be in exactly the same energy state
Hund’s Rule: the rule that states that for an atom in the ground state, the number of unpaired electrons is the maximum possible and these unpaired electrons have the same spin
Noble Gases: Noble Gases are all of the elements in the 18th period and they are Helium, Neon, Argon, Krypton, Xenon, and Radon.
ORBITALS: High probability regions where electrons are likely to be found
S (1)
P (3) Filling order for atoms with more than one electron
D (5)
F (7)
Louis de Braglie: -“Inventor” of quantum mechanics
-“Electrons, like light, exhibit particle wave duality”
-any object exhibits particle/wave duality, but more massive
objects tend to behave more like particles
Light exhibits particle and wave duality
Light as Wave:
Constructive Interference: 2 waves that have curtain height to add together to make a bigger wave Destructive Interference: no light; waves cancelling each mother out --Double Slit experiment
Electromagnetic Radiation- A form of energy that exhibits wavelike behavior as it travels through space
Quantum-Energy is the minimum quantity of energy that can be lost or gained by an atom.
Wavelength- λ-The distance between corresponding points on adjacent waves.
Frequency- ν-Defined as the number of waves that pass a given point in a specific time, usually one second. (wave/second) 1 w/s=Hertz
Speed of light: 3.00 x 108 meters/second
Frequency & Wavelength relationship:
Speed of light= wavelength X frequency
Photoelectric effect- Refers to the emission of electrons from a metal when light shines on the metal
Planck’s Constant: 6.626 x 10-34 Joules x Seconds
Relationship between a quantum of energy and frequency of radiation:
Energy= Planck’s constant X Frequency
Photon- A particle of electromagnetic radiation having zero mass and carrying a quantum of energy
When a narrow beam of the emitted light was shined through a prism, it was separated into 4 specific colors of the visible spectrum. 4 bands of lights were part of hydrogens line-emission spectrum.
Continuous Spectrum- The emission of a continuous range of frequencies of electromagnetic radiation.
Bohr Model:
· Electrons can have only certain energies
· Colors are emitted when electrons jump from higher to lower energy levels
Aufbau Principle: the principle that states that the structure of each successive element is obtained by adding one proton to the nucleus of the atom and one electron to the lowest-energy orbital that is available
Pauli Exclusion Principle: the principle that states that two particles of a certain class cannot be in exactly the same energy state
Hund’s Rule: the rule that states that for an atom in the ground state, the number of unpaired electrons is the maximum possible and these unpaired electrons have the same spin
Noble Gases: Noble Gases are all of the elements in the 18th period and they are Helium, Neon, Argon, Krypton, Xenon, and Radon.
ORBITALS: High probability regions where electrons are likely to be found
S (1)
P (3) Filling order for atoms with more than one electron
D (5)
F (7)
Louis de Braglie: -“Inventor” of quantum mechanics
-“Electrons, like light, exhibit particle wave duality”
-any object exhibits particle/wave duality, but more massive
objects tend to behave more like particles
Light exhibits particle and wave duality
Light as Wave:
Constructive Interference: 2 waves that have curtain height to add together to make a bigger wave
Destructive Interference: no light; waves cancelling each mother out
--Double Slit experiment
Light as Particle:
--Paddle-wheel experiment
--Photoelectric effect
What is the Electron Configuration for Oxygen?
What is the Electron Configuration for Vanadium?
A.1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 4d3
B. 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d3h
C. 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 4d4
What is the Orbital Diagram for Oxygen?
→
B
What is the Orbital Diagram for Nitrogen?
→
B
What is the Noble Gas configuration for Sodium?
- [Ar] 3s2, 3p6
- [Ar] 3p6
- [Ne] 3s1
- [Ne] 3s2, 3p6
What is the Noble Gas configuration for Carbon?- [Ne] 2s2, 2p6
- [He] 2s2, 2p2
- [Ne] 3s2, 3p6
- [He] 2s2, 2p6
Determine the wavelength of a wave broadcasted by 93.7 MHz.93.7 MHz (106 Hz/1MHz) = 93700000Hz
(3.00*108 m/s / 93700000Hz) = 3.20 M